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Name ………………………………….class……………teacher………….date ……………

1) The chemical formula for tetrachloromethane is CCl4. What is the relative molecular mass of tetrachloromethane? [Relative atomic mass: C, 12; Cl, 35.5]

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2) The following equation shows the reaction between silver nitrate and sodium chloride. AgNO3(aq) + NaCl(aq) → AgCl(s) + NaNO3(aq)

What is the mass of the insoluble salt produced when 50 cm3 1.0 mol dm-3 silver nitrate reacts with 50 cm3 2.0 mol dm-3 sodium chloride? [Realtive atomic mass : N = 14, O = 16, Na = 23, Cl = 35.5, Ag = 108]

………………………………………………………………………………………………………3) Aluminium carbonate decomposes when heated strongly to produce aluminium oxide and carbon dioxide.

Al2(CO3)3 Al2O3 + 3CO2

What is the maximum volume of the gas that can be obtained at room temperature when 23.4 g of aluminium carbonate is heated?[ Molar mass of Al2(CO3)3 = 234 g mol-1 ; Molar volume of gas at room temperature = 24 dm3 mol-1]

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Pair of metalsPasangan logam

Potential difference (V)Beza upaya (V)

Negative terminalTerminal negatif

R and copperR dan kuprum

0.44 R

S and copperS dan kuprum

1.70 S

T and copperT dan kuprum

0.53 Cu

What is the potential difference for the pair of metal S and T?

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5) In an experiment, 24 g of element X react with 32 g sulphur to form a compound. What is the empirical formula of that compound ? [Relative atomic mass ; X = 6, S = 32 ]

………………………………………………………………………………………………………………6) A compound contains 2.56g copper and 0.64g oxygen Determine the empirical formula of the compound Q.

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7) The empirical formula of compound L is C2H5. Determine its molecular formula given that the relative molecular mass is 58.[Relative atomic mass: C=12; H=1]

…………………………………………………………………………………………………………8) The chemical equation for the reaction is:

H2SO4 + 2KOH K2SO4 + 2H2O

What is the volume of 0.1 mol dm-3 sulphuric acid needed to exactly neutralize 20 cm3 0.1 mol dm-3 potassium hydroxide?

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9) Distilled water is added to 20.0 cm3 of solution 0.1 mol dm-3 of Z to make 100.0 cm3 of solution.Calculate the new concentration of solution Z.

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10) The equation represents a neutralization reaction.

2HNO3 + Ba(OH)2 → Ba(NO3)2 + 2H2O

10.0 cm3 of barium hydroxide solution 0.1 mol dm-3 is titrated with nitric acid 0.1 mol dm-3. If the initial reading of the burette is 10.00 cm3, what is the final reading of the burette?

…………………………………………………………………………………………………….11) 25 cm3 of 0.1 mol dm-3 sodium hydroxide solution is required to react completely with 12.50 cm3 of dilute hydrochloric acid.

Calculate the molarity of the dilute hydrochloric acid used.

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12) Diagram 22 shows the energy level diagram for neutralisation reaction.

What is the amount of heat released when 50 cm3 2 mol dm-3 sulphuric acid reacts with 50 cm3 2 mol dm-3 potassium hydroxide solution?

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Reaction path

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13) The reaction between sodium and chlorine forms a compound with a high melting point.. Determine the mass of the compound formed when 2.3 g sodium reacts with excess chlorine.

[Relative atomic mass Na= 23, Cl= 35.5]

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14) Calculate the oxidation number of i) Manganese in KMnO4

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ii) chromium in Cr2O7 2-- ion.

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15) The following chemical equation shows the reaction between calcium carbonate and hydrochloric acid.

Determine the mass of calcium carbonate needed in the reaction if 480 cm3 of gas is released at room condition. (The molar volume of gas at room condition: 24 dm3 mol-1, Relative atomic mass: C = 12 g, O= 16 g, Ca = 40 g)

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16) The volume of gas released is recorded in Table 7.1

Time / sMasa/ s 0 60 120 180 240 300 360

Volumeof gas / cm3

Isipadugas / cm3

ExperimentI 0.00 25.90 33.00 37.00 40.50 42.00 42.00

Experiment II 0.00 28.00 36.50 41.00 42.00 42.00 42.00

Based on the graph, determine (i) The average rate of reaction for the whole experiment

(ii) The average rate of reaction for the first 2 minutes

(iii) the rate of reaction at 90 sec for Experiment I. ( how?)

2HCl + CaCO3 CaCl2 + CO2 + H2O

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17)

(Relative atomic mass: N=14, O=16, Cu=64, molar volume of gas at room condition; 24 dm3 mol-1)

(i) Determine the percentage composition by mass of oxygen in copper(II) nitrate.

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ii) If 3.2 g of copper(II) oxide is produced during the heating process, calculate the volume of oxygen gas evolved at room condition.

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18) Diagram 10 shows an energy level diagram.

Diagram 10.1

Determine the temperature change when 50 cm3 of 1.0 mol dm-3 of hydrochloric acid reacts with excess magnesium. [Specific heat capacity of solution: 4.2 J g-1 o C-1,

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In this experiment, 5 g excess copper is added to 100 cm3 of 0.5 mol dm-3 silver nitrate solution. The heat of displacement in this experiment is -105 kJmol-1. [ Specific heat capacity of the solution is 4.2 Jg-1oC-1 ; the density of the solution is 1.0 gcm-3 ]

(i) Calculate the heat energy released in this experiment.

……………………………………………………………….ii) Calculate the temperature change in this experiment.

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2 Cu(NO3)2 2 CuO + 4 NO2 + O2

EnergyTenaga

Mg + 2 HCl

Mg Cl2 + H2

ΔH = -50.4 kJ mol -1

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20) 50 cm3 of hydrochloric acid neutralize 50 cm3 of sodium hydroxide. Initial Temperature of HCl is 29.0 o C, Initial temperature of NaOH is 29.5 oC. Highest temperature of the mixture is 36.0 oC. Calculate heat of neutralization [ Specific heat capacity of the solution is 4.2 Jg-1oC-1 ; the density of the solution is 1.0 gcm-3 ]

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21) 4.6 g of ethanol is needed to heat 500 cm3 of water . Increase in temperature of water is 30 oCMolar mass of ethanol is 46 gmol-1. Calculate the heat of combustion of ethanol [ Specific heat capacity of the

solution is 4.2 Jg-1oC-1 ; the density of the solution is 1.0 gcm-3 ]

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22) Diagram 3 shows the energy profile for the reaction between X and Y to produce Z.

i) What is the activation energy of the reaction and the type of reaction? …………………………………..

ii) What is the heat of reaction for this reaction?

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23) Carbon burns in oxygen in a reaction as shown in the equation below.

C(s) + O2(g) CO2 (g) ▲ H = -394 kJ mol-1

What is the mass of carbon that must be burnt completely to produce 78.8 kJ of heat?

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Based on the diagram above, i) state the volume of barium

chloride solution 0.5 mol dm-3 for reacts completely with 5 cm3 of potassium chromate(VI) solution

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………………………………………………..ii) calculate the number of mole of barium chloride solution is needed to reacts completely with 1 mole potassium

chromate(VI) solution.

………………….work hard- work smart!!